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(B) Pauli's Exclusion Principle states that no two electrons in an atom can have the same set of all four quantum numbers. This implies that an orbita

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Only $C$

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(B) Pauli's Exclusion Principle states that no two electrons in an atom can have the same set of all four quantum numbers. This implies that an orbital can hold a maximum of two electrons,and if it does,they must have opposite spins (represented by arrows pointing in opposite directions).Analyzing the given diagrams:- $(A)$: All orbitals follow the rule. The third orbital has two electrons with opposite spins.- $(B)$: The third orbital has two electrons with the same spin (both pointing down). This violates Pauli's Exclusion Principle.- $(C)$: All orbitals follow the rule.- $(D)$: The first orbital has two electrons with opposite spins. The other orbitals are correctly filled according to Hund's rule. This does not violate Pauli's Exclusion Principle.Therefore,only diagram $(B)$ violates Pauli's Exclusion Principle. However,looking at the provided options,there might be a misinterpretation of the diagram $(B)$'s third box or $(D)$'s first box. Re-evaluating: In $(B)$,the third box shows two electrons with the same spin (both down),which is a violation. In $(D)$,the first box shows two electrons with opposite spins,which is correct. Thus,only $(B)$ violates the principle. Given the options,if $(B)$ is the only violator,the question might be flawed or the options provided are limited. Based on standard interpretation,only $(B)$ violates the principle.

The portion of orbital diagrams representing the electronic configuration of certain elements is shown below. Which of them violate Pauli's Exclusion principle?

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